Want this question answered?
A solution of HCl is highly dissociated into ions, A 0.000001 M solution (1 x 10-6) has a pH of 6 ... close to neutral. A 0.001 M solution (1 x 10-3) has a pH of 3 ... more concenterated, but still not a really concentrated solution. A 0.1 M solution (1 x 10-1) has a pH of 1 ... even more concentrated. showing it is more acidic.
For the preparation of a solution with the pH=7,00:Add 29,1 mL sodium hydroxide solution 0,1 M to 50 mL potassium dihydrogen phosphate solution 0,1 M.
pH = -log [H+], so if the [H+] is 2.310 M, the pH = -0.3636
pOH= -log(0.0220M OH) pH=14-pOH pH=12.34242268
[H+] = 1 x 10-10 M then pH = 10
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
its PH is 3
- log(0.12 M) = 0.92 pH ---------------
-log(0.5 M HF) = 0.3 pH
- log(0.000626 M H2SO4) = 3.2 pH -----------
A 0.01 M solution of NaOH has a pH =13
Its pH value is 2.
For example, to obtain a solution with the pH=7,00 mix: 756 mL 0,1 M solution of Na2HPO4 with 244 mL of 0,1 M HCl solution.
A 1.0 M aqueous solution has a pH of 11.6
11.45
13.51
- log(0.01 M HNO3) = 2 pH =====